For the reaction, I 2(g) leftharpoons 2 I (g) ; KC=37.6 × 10-6 at 1000 K. If 1.0 mole of I 2 is introduced into a 1.0 L flask at 1000 K, at equilibrium

Question

For the reaction, I 2(g) leftharpoons 2 I (g) ; KC=37.6 × 10-6 at 1000 K. If 1.0 mole of I 2 is introduced into a 1.0 L flask at 1000 K, at equilibrium (A) [ I 2]>[ I ] (B) [ I 2]=[ I ] (C) [ I 2]<[ I ] (D) Unpredictable

Tardigrade Admin · Accepted Answer

As KC is very low and KC=([ I ]2/[ I 2]) For the reaction, I 2(g) leftharpoons 2 I (g) ∴ [ I 2]>[ I ]

Q. For the reaction,
$I_{2} (g) ⇌ 2 I (g); K_{C} = 37.6 \times 1 0^{- 6}$
at $1000 K$ . If $1.0$ mole of $I_{2}$ is introduced into a $1.0 L$ flask at $1000 K$ , at equilibrium

$[I_{2}] > [I]$

$[I_{2}] = [I]$

$[I_{2}] < [I]$

Unpredictable

As $K_{C}$ is very low and $K_{C} = \frac{[ I ] ^{2}}{[ I _{2} ]}$
For the reaction, $I_{2} (g) ⇌ 2 I (g)$
$∴ [I_{2}] > [I]$

Q. For the reaction, I2​(g)⇌2I(g);KC​=37.6×10−6 at 1000K. If 1.0 mole of I2​ is introduced into a 1.0L flask at 1000K, at equilibrium

[I2​]>[I]

[I2​]=[I]

[I2​]<[I]